For the reaction $A + B \to C$, it is found that doubling the concentration of $A$ increases the rate by $4$ times, and doubling the concentration of $B$ doubles the reaction rate. What is the overal order of the reaction.

If reaction between $A$ and $B$ to give $C$shows first order kinetics in $A$ and second order in $B$, the rate equation can be written as

Consider the following single step reaction in gas phase at constant temperature.

$2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})}$

The initial rate of the reaction is recorded as $r_1$ when the reaction starts with $1.5 \mathrm{~atm}$ pressure of $\mathrm{A}$ and $0.7 \mathrm{~atm}$ pressure of B. After some time, the rate $r_2$ is recorded when the pressure of $C$ becomes $0.5 \mathrm{~atm}$. The ratio $r_1: r_2$ is $\qquad$ $\times 10^{-1}$.

(Nearest integer)

Hydrolysis of methyl acetate in aq. solution has been studied by titrating the liberated acetic acid against solidum hydroxide. The conc. of the ester at different time is given below :

Show that it follows a pseudo first order reaction as the conc. of  $H_2O$ remain nearly constant $(54.2\,mol\,L^{-1})$ during the course of the reaction. What is the value of $k'$ in this reaction ?

For the following reaction scheme (homogeneous), the rate constant has units

$A+B\xrightarrow{K}C$:

In the hydrolysis of an organic chloride in presence of large excess of water
$RCl + H_2O \longrightarrow ROH + HCl$